Chemistry Chapter 14 Acid Review

Acids and Bases

• Acids react with bases to form salt and water, releasing hydrogen ions (H+).
• Binary acids consist of hydrogen and another electronegative element, e.g., Hydrochloric acid (HCl).
• Common binary acids include Hydrofluoric, Hydrochloric, Hydrobromic, Hydriodic, and Hydrosulfuric.

Types of Acids

• Oxyacids contain hydrogen, oxygen, and another nonmetal element.
• Strong acids include HI, HCl, HBr, H2SO4, and HNO3, known for complete ionization in solution.
• Weak acids, such as transitional bases, do not fully dissociate, retaining some hydrogen.

Acid and Base Strength

• The strength of bases depends on their ability to dissociate and release hydroxide ions (OH-).
• Bronsted-Lowry acids donate protons, while Bronsted-Lowry bases accept protons.
• Lewis acids accept electron pairs, while Lewis bases donate electron pairs.

Acid-Base Reactions

• In Bronsted-Lowry reactions, protons transfer from acids to bases, forming conjugate bases and acids.
• Neutralization reactions between acids and bases produce salt and water, occurring at equal concentrations of hydrogen and hydroxide.

Properties of Acids and Bases

• Acids typically have a sour taste and many release hydrogen gas when reacting with active metals.
• Aqueous solutions of acids can conduct electricity.
• Bases have a bitter taste and feel slippery.

Naming and Identifying Acids

• Binary acids are identified by the prefix "hydro-"; oxyacids do not use this prefix.
• Acid names with the suffix -ic correspond to anions with the suffix -ate, while those with -ous have fewer oxygen atoms.
• Sulfuric acid is the most produced acid globally, while hydrochloric acid is used for pickling metals and in the stomach.

Key Applications of Specific Acids

• Sulfuric acid is used in batteries and the manufacture of explosives and fertilizers.
• Phosphoric acid is utilized in food flavoring and detergent production.
• Acetic acid, which gives vinegar its flavor, is found in many culinary uses.

Historical Context

• The Arrhenius theory established the definitions of acids and bases, focusing on ion concentration in aqueous solutions.
• An Arrhenius acid is characterized by an increase in hydrogen ions when dissolved in water, while an Arrhenius base does the same for hydroxide ions.